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24 Cards in this Set
- Front
- Back
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Bonding
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- How atoms interact depending on their electron configurations
- Valence e- are the only things we care about here |
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Formal Charges
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FC = V - ½B - L
- Tells us the electron configuration of each atom in a compound. - Best configuration of bonds is when FC=0, or when the charge is the least |
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Resonance
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- "Average" of Formal charge
- Determined through experiments determining the bond length |
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Covalent Bond
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- "Sharing" of electrons between valence electrons of two atoms
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Polar Covalent Bond
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- Polarity is when one atom has a greater electron density concentrated around it than another.
- Greater difference in electronegativity, the greater dipole moment |
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Coordinate Covalent
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- When one atoms shares both of its unshared pair of electrons, the bond breaks and the electrons leave
- A Lewis Base donates a pair of electrons to a lewis acid! |
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Ligand
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- Lewis Base
- Donates both electrons to make a coordinate covalent bond |
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Ionic Bonds
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- Bonds held together by an electrostatic attraction between a cation and an anion
- qq/r |
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Ion-Dipole
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- Polar molecule attracted to ions
- Basically between a +/- charge and a dipole |
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Dipole-Dipole
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- Between two polar molecules
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Hydrogen Bonding
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- Special form of dipole-dipole
- Between a "H-Bond Donor" and an "H-Bond Acceptor". - H Bond donors: N, O, F, H - H Bond acceptors: N, O, F, lone pair - Increases BP significantly |
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Ranks of Bonding Strengths
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Covalent Bonds > Ionic > Ion-Dipole > Dipole-Dipole (H-Bonds) > London Dispersion
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London Dispersion
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- Instantaneous dipoles induced in two neighboring nonpolar molecules
- "Default" force that is always there - Think gases at room temperature |
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Vespr Theory
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- Shapes of molecules depicted by set model
- Since electrons repel each other, they want to be as far away as possible |
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Geometric Family
2 Electron Groups |
Linear
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Geometric Family
3 Electron Groups |
Trigonal Planar
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Geometric Family
4 Electron Groups |
Tetrahedral
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Geometric Family
5 Electron Groups |
Trigonal Bipyrimidal
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Geometric Family
6 Electron Groups |
Octahedral
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With ONE pair of lone e-
What are the shapes of 3,4,5,6? |
- 3: Bent
- 4: Trigonal Pyramid - 5: See-saw - 6: Square Pyramidal |
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With TWO pairs of lone e-
What are the shapes of 4,5,6? |
- 4: Bent
- 5: T-Shape - 6: Square Planar |
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Ionic Solids
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- Held together by electrostatic attractions between cations and anions in lattice structure
- Solids are ionic if their electronegativity is different - Strongest, solid at RT |
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Network Solids
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- Covalent bonds make a lattice
- One big molecule, very strong, very hard at room temperature - Example: Diamond, Quartz |
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Metallic Solids
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- "Cloud" of valence electrons move through the solid
- Good conductors of heat and electricity |
